yes
No. It has polar bonds but they are distributed equally in the molecule so it, as a whole, isnt polar.
Sulfur dibromide is a bent molecule. In general bent molecules are polar. The situation is a bit complex with SBr2 - when looking at each S-Br bond the difference in electronegativity is small. Bromine is slightly more electronegative than sulfur - so you can think of this bond as either non-polar covalent OR slightly polar. If you draw a vector in the direction of the partial charges (dipoles going from sulfur - to bromine) there will be a very slight polarity. The polarity is very small and since S-Br bonds are typically considered non-polar, many people classify SBr2 as a non-polar molecule since the dipole is very small.
SO2 is the substance that has polar covalent bonds. This is because sulfur and oxygen have different electronegativities, resulting in an uneven sharing of electrons in the covalent bonds within the molecule.
The SCl2 molecule is polar because it has a bent molecular geometry with two chlorine atoms that have greater electronegativity than sulfur, resulting in an unequal sharing of electrons and creating a net dipole moment.
NF3 is a polar covalent molecule. While the electronegativity difference between N and F suggests more ionic character, the shape of the molecule (trigonal pyramidal) results in an uneven distribution of charge, making it polar covalent.
The bond in the molecule is covalent.
No. It has polar bonds but they are distributed equally in the molecule so it, as a whole, isnt polar.
BeF2 is non-polar as it is (strangely) covalent in nature and as such, the molecule has a linear shape which produces a non-polar molecule.
SO2 is the substance that has polar covalent bonds. This is because sulfur and oxygen have different electronegativities, resulting in an uneven sharing of electrons in the covalent bonds within the molecule.
Sulfur dibromide is a bent molecule. In general bent molecules are polar. The situation is a bit complex with SBr2 - when looking at each S-Br bond the difference in electronegativity is small. Bromine is slightly more electronegative than sulfur - so you can think of this bond as either non-polar covalent OR slightly polar. If you draw a vector in the direction of the partial charges (dipoles going from sulfur - to bromine) there will be a very slight polarity. The polarity is very small and since S-Br bonds are typically considered non-polar, many people classify SBr2 as a non-polar molecule since the dipole is very small.
It is a non-polar molecule. But it has polar covalent bonds between its atoms
The SCl2 molecule is polar because it has a bent molecular geometry with two chlorine atoms that have greater electronegativity than sulfur, resulting in an unequal sharing of electrons and creating a net dipole moment.
Carbon dioxide is a non-polar molecule containing polar covalent bonds in its atoms.
carbon dioxide
not necessarily. if the individual dipoles cancel off, then the molecule will be non-polar. As in CCl4, PCl5 etc
NF3 is a polar covalent molecule. While the electronegativity difference between N and F suggests more ionic character, the shape of the molecule (trigonal pyramidal) results in an uneven distribution of charge, making it polar covalent.
Sulfur hexafluoride has covalent bonds.